In thermodynamic of the dissolution of Borax lab, the student's graph is below. CalculateAS? (R= 8.314 x 10-3 kJ/mole K)LN of Ksp vs 1/Temperature in KelvinLN Ksp00.0031 0.0032 0.00330.00340.0035 0.0036 0.0037-2-4-6y=-9104.5x + 26.39R2 = 0.9713Temperature in K-1Series1.........Linear (Series1)OA) 0.008075 kJ/mol KB) -75.69 kJ/mol KOC) -0.008075 kJ/mol KOD) -0.2194 kJ/mol KOE) 75.69 kJ/mol KOF) 0.2194 kJ/mol K

Step 1: To get ΔS we'll need to identify the intercept and R. Both are given is in question where…

Answered: In thermodynamic of the dissolution of…

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter13: Electrochemistry

Section: Chapter Questions

Problem 13.90PAE: A chemical engineering student is studying the effect of pH on the corrosion of iron. Ellie...

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Reaction KspKsp ΔH°ΔH° ΔS°ΔS° FeCO3(s)⇄Fe2+(aq)+CO32−(aq)FeCO3(s)⇄Fe2+(aq)+CO32−(aq) 3×10−113×10−11 <0<0 >0>0 MnCO3(s)⇄Mn2+(aq)+CO32−(aq)MnCO3(s)⇄Mn2+(aq)+CO32−(aq) 2×10−112×10−11 <0<0 >0 The table above lists the equilibrium constants and changes in thermodynamic properties for the dissolution of FeCO3 and MnCO3 at 25°C. The two-particle diagrams below represent saturated solutions of each compound at equilibrium. (see attached image) a.) The particle diagrams best represent that ΔH°<0ΔH°<0 because the ions from both compounds are solvated by water molecules. b.) The particle diagrams best represent that ΔH°<0ΔH°<0 because both compounds produce about the same amount of CO32−CO32− ions from the dissolution. c.) The particle diagrams best represent that ΔS°>0ΔS°>0 because both compounds produce a very small amount of ions from the dissolution. d.) The particle diagrams best represent that the molar solubility is greater for…
What is Ecell at 25°C for the reaction Ca(s) | Ca2+(2.898 M) || Sn2+(0.137 M) | Sn(s)? Report your answer to the hundredths place and do not include units. Half-reaction E° (V) Ca2+ + 2e- → Ca(s) -2.87 Sn2+ + 2e- → Sn(s) -0.14
In Fe + O2 --> Fe2O3 what is the coefficient for Fe?
Some wastewater stream contains 0.015 M Hg22+. Some chemical engineer decides to remove it by precipitating it as Hg2CO3(s). He mixes 100.00 ml of the wasterwater with 100.00 ml of a 2.00 M solution of Na2CO3 and filters the result to remove the solid. How much residual Hg22+ should he expect to find still in the water? (Hint: it should not be 0) Ksp of. Hg2CO3 = 9.0 x 10-15. Also keep in mind that Hg+ is the only ion that exists in solutions as a dimer, i.e. Hg22+, not 2 Hg+ (Hg2CO3→ Hg22+ + CO32-)
Potassium dichromate has several industrial applications. To determine the purity of the salt that will be used in different industrial processes, a sample mass equal to 2.660 g was dissolved and quantitatively transferred to a 500.00 mL flask. An aliquot of 25.00 mL of this solution was treated with excess KI and the released iodine was titrated with 0.1000 mol L-1 sodium thiosulfate, spending 27.00 mL. Calculate the purity of the analyzed salt. Data:K = 39.10 O = 16.00 Cr = 52.00 I = 126.9 S = 32.07
A chemical engineering student is studying the effect of pH on the corrosion of iron. Ellie following data are collected: Corrosion Rate (mm/year) ph 0.03 13.00 0.06 12.00 0.16 11.00 0.22 10.00 0.25 9.00 0.25 8.00 0.25 7.00 0.25 6.00 0.25 5.00 0.27 4.00 0.37 3.00 0.38 2.80 0.63 2.80 1.00 2.80 Plot corrosion rate vs. pH. (HINT: Label the x axis with decreasing pH.) (a) How would you describe the dependence of corrosion on pH? (b) When the pH goes below 3, bubbles appear in the solution. What change takes place in the reduction half-reaction at low pH? (c) How do you explain the shape of the curve at the lowest pH? (Based on a graph in the Kirk-Otbmer Encyclopedia of Chemical Technology, 4th ed., vol 7. New York: John Wiley & Sons, p. 559.)
Calculate the solubility of lead(II) sulfate (Ksp = 2.53x10-8) in a 0.0034 M solution of sodium sulfate. Give your answer to three sig. figs. and in exponential form (e. g. 1.23E-3).
Given that E° = +0.897 V, calculate E at 25°C forPb(s) ∣ Pb2+(0.0400 M) ∣∣ Fe3+(0.200 M), Fe2+(0.0100 M) ∣ Pt(s) A) +0.779 VB) +0.935 VC) +1.015 VD) +1.134 V Thank you!
Thermodynamics Quantities for Selected Substances at 298.15 K (25⁰C) Substance ∆H⁰f (kJ/mol) ∆G⁰f (kJ/mol) S (J/K-mol) Hydrogen H2(g) 0 0 130.58 Oxygen O2(g) 0 0 205.0 H2O(l) -285.83 -237.13 69.91 10. What is the ∆S⁰ in the combustion of hydrogen in the presence of excess oxygen yields water: 2H2(g) + O2(g) → 2H2O(l) in J/K?
Given: MnS + H+ < -- > Mn2+ + HS- CuS + H+ < -- > Cu2+ + HS- [A] Classify each reaction as exothermic or endothermic based on the DGr0 (Gibbs energy in kJ/mol). [B] What is the Ksp of MnS and CuS? [C] Which is more soluble? Gibbs free energy given in kJ/mol: CuS = −86.2 MnS = 30
Thermodynamics Quantities for Selected Substances at 298.15 K (25⁰C) Substance ∆H⁰f (kJ/mol) ∆G⁰f (kJ/mol) S (J/K-mol) Carbon C2H2(g) 226.7 209.2 200.8 C2H4(g) 52.30 68.11 219.4 Hydrogen H2(g) 0 0 130.58 Oxygen O2(g) 0 0 205.0 H2O(l) -285.83 -237.13 69.91 3. What is the value of ∆S⁰ for the catalytic hydrogenation of ethene to ethane: C2H4(g) + H2(g) → C2H6(g) + 2H2O(l) in J/K?
For the reaction pictured, the experimental enthalpy is -41.3 ± 1.3 kJ mol-1. When using the Gaussian command line # B3LYP/6-31G(d) opt freq int=grid=ultrafine, the enthalpy was -40.1, but when using the Gaussian command line # MP2/cc-pVTZ scf=tight, the enthalpy was -42.4. What would cause one method to be more accuarate than the other? Thank you :)

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